At constant pressure,the combustion of 5.00 g of C₂H₆(g) releases 259 kJ of heat.What is ΔH for the reaction given below?
2 C₂H₆(g) + 7 O₂(g) → 4 CO₂(g) + 6 H₂O(l)

Question

At constant pressure,the combustion of 5.00 g of C₂H₆(g)releases 259 kJ of heat.What is ΔH for the reaction given below? 2 C₂H₆(g)+ 7 O₂(g)→ 4 CO₂(g)+ 6 H₂O(l)

Quizplus · Accepted Answer

The combustion of 5.00 g of C2H6 releases 259 kJ. The molar mass of C2H6 is 30.07 g/mol, so 5.00 g corresponds to 5.00/30.07 = 0.166 mol. The reaction involves 2 moles of C2H6, so ΔH for the reaction is (259 kJ / 0.166 mol) * 2 = -3120 kJ.

At Constant Pressure,the Combustion of 5